The density of molten copper at 1200 0C is near 7,898 g/cm3. An empirical formula is: d (g/cm3) = 9,077 - 8,006.10-4 T (in K)
Water at 4°C (39°F) has a density of 1.
Elasticity and Density of the medium c^2=elasticity/density
At standard pressure (100 kPa), dry air at 0 °C has a density of 1.2754 kg/m3 or 1.2754 g/L. Changing the composition, pressure, temperature or humidity changes the density.
The density of water at 27.3 degrees C is 0.996429 g/cm3.
Short Answer:Water reaches it maximum density at 3.98 °C (39.16 °F).The density of ice 0.9168 g/cm3 at 0 °C .The density of water, 0.99984 g/cm3 at 0 °C and 0.99997 g/cm3 at 4 °C.Explanation:Water gets more dense as it cools until it reaches 4 degrees C. At that point, because water molecules (and the forces between them) are not spherical, they begin to exhibit a tendency to hold particular orientations at preferred separation distances that keep them further apart than was possible above 4 C. Cooling from 4 C towards 0 C removes more kinetic energy allowing the preferred orientations and separations to become more orderly, further decreasing density. At freezing, 0 C, the nonspherical forces between molecules lock them into the preferential orientations and separations of the ice crystal arrangement with a sharp increase in average separation and decrease in bulk density.Water is at its greatest density at 3.98 degrees CentigradeWater is at its maximum density at 4 oC.
copper's melting point is 1,083°C and its boiling point is 2,595°C just for fun A coin is usually, made of copper or a copper alloy. But the question was what temperature does it burn at - I'd like to know too - when copper is molten it's surface emits a blue flame, which is presumably burning copper, this happens as soon as it melts.
All the silicates are molten at about 1200°C and all are solid when cooled to about 600°C.
Molten lava near the surface can reach 1200 deg. C, or 2200 deg. F.
Density
1200 Celsius = 2192 Fahrenheit .
The mass of copper is 240 g.Use the following formula:q = m x c x DeltaT,where:q is energy, m is mass, c is specific heat capacity, and DeltaT is the change in temperature.DeltaT = Tfinal-TinititalKnownq = 1200 calcCu = 0.0923 cal/g.oCTinitial = 20oCTfinal = 75oCDeltaT = 75oC - 20oC = 55oCUnknownmass of copperSolutionRearrange the equation q = m x c x DeltaT to isolate m. Plug in the known values and solve.m = q/(c x DeltaT)m = 1200/(0.0923 x 55) = 240 g (rounded to two significant figures)
Assumed as a single copper busbar and not considering the length: @ 30°C = 1403 Amps. @ 35°C = 1355 Amps. @ 40°C = 1306 Amps. @ 45°C = 1255 Amps.
Copper Loss at 75 C = Copper Loss at Ambient Temperature C * (310/(235+Ambient Temperature C))
1200 c
The temperature 800°C (which is the same as 1472°F) is much hotter than the temperature of molten lead or zinc, but not hot enough to melt copper, gold, or silver. The red part of a candle flame is about 800°C, while the blue part is hotter (1400°C).
Density @ 15 Deg = 0.7952 ( 20 Deg Density + 0.0032)
Copper has a CTE of 16.6 parts per million/degree C (16.6E-6/C)